Worksheet: Osmotic Concentration

In this worksheet, we will practice describing how dissociation affects osmosis and converting osmotic pressures to molar concentrations.

Q1:

The osmotic pressure of human blood is 7.6 atm at 37C. What mass of glucose, CHO6126, is required to make 1.00 L of aqueous solution for intravenous feeding if the solution must have the same osmotic pressure as blood at body temperature, 37C?

Q2:

A 0.010 M solution of the weak acid HA has an osmotic pressure of 0.293 atm at 25C. A 0.010 M solution of the weak acid HB has an osmotic pressure of 0.345 atm under the same conditions. Each solution contains three dissolved species: the weak acid (HA or HB), the conjugate base (A or B), and the hydrogen ion (H+). The osmotic pressure of each solution is related to the solute concentrations in molar units.

Which acid has the larger equilibrium constant for ionization? HAHA()A()+H()HBHB()H()+B()()()aqaqaqaqaqaq++

  • A H A
  • B H B

What is the equilibrium constant for the ionization of HA?

  • A 4 × 1 0
  • B 6 × 1 0
  • C 3 × 1 0
  • D 5 × 1 0
  • E 3 × 1 0

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